# A certain half-reaction has a standard reduction potential E-=-0.77 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell thamust provide at least 1.30 V of electrical power. The cell will operate under standard conditions.Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cellIs there a minimum standard reduction0=vyes, there is a minimum.Epotential that the half-reaction used atredthe anode of this cell can have?If so, check the "yes" box and calculatethe minimum. Round your answer to 2decimal places. If there is no lowerlimit, check the "no" boxXno minimumIs there a maximum standard reduction0Ered3 ПvO yes, there is a maximumpotential that the half-reaction used atthe anode of this cell can have?If so, check the "yes" box and calculatethe maximum. Round your answer to 2mal places. If there is no upperlimit, check the "no" boxno maximumBy using the information in the ALEKSData tab, write a balanced equationdescribing a half reaction that could beused at the anode of this cellNote: write the half reaction as it wouldactually occur at the anode. Ag (aq)e- Ag (s)Al3+ (aq) 3e Al (s)0.7996-1.676Au (aq) e" Au (s)1.692Au3+ (aq) 3eAu (s)1.498Ba2+ (aq)2eBa (s)-2.912Br2 ()2e - 2Br (aq)1.066Ca2+ (aq)2e -- Са (s)-2.868Cl2 (g)2e » 2Cl (aq)1.35827Co2+ (aq) 2eCo (s)-0.28Co3+ (aq) e- Co2+ (aq)1.92Cr2+ (aq) 2eCr (s)-0.913Cr3+ (ag) 3e Cr (s)-0.744Cr3+ (aq) e- Cr2+ (aq)-0.407CrO42- (aq) 4H20 (I) +3eCr(OH)3 (s)50H- (aq)-0.13Cu2+ (aq)2e-Cu (s)0.3419Cu2+ (aq) e Cu (aq)0.153Cu (aq)e-Cu (s)0.521F2 (g)2e 2F (aq)Fe2+ (aq)2e2.866Fe (s)-0.447Fe3+ (aq)e"- Fe2+ (aq)0.771Fe3+ (aq) 3eFe (s)-0.0372H+ (aq) 2eH2 (g)0.0002H20 ()2e- H2 (g) + 20H (aq)-0.8277

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Step 1

The relation (1) provides the formula for calculating the electrode potential of a cell and the relation (2) describes the dependence of the standard free energy change on the standard cell potential. In these equations, E0cell is used for standard cell potential, E0c is used for the standard reduction potential at the cathode, E0a is used for the standard reduction potential at the anode, n is the number of electrons transferred, F is Faraday’s constant and ΔG is the standard free energy change.

Step 2

(i)

For a reaction to be spontaneous, the free energy change of the reaction must be negative. From equation (2), the value of standard free energy change will be negative, if the value of standard cell potential is positive. Therefore, the value of E0cell should be positive for a reaction to be spontaneous.

For the given galvanic cell, the electrode potential of the cell should be atleast 1.30 V and the reduction potential at the cathode is -0.77 V.

For this reaction to be spontaneous, there will be no minimum value for the reduction potential at the anode because a greater magnitude of negative value of E0a leads to the increase in positive value of E0cell as per the relation given in equation (1).

Step 3

(ii)

The maximum value for the electrode potential at the ano...

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